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As the definition of a Lewis acid says:
"Capable of accepting electron pair (from a (Lewis) base".
So H+ and Ag+ are both Lewis acids compared in the following reaction with ammonia:
(in which the N-atom is donating the unbound electron pair as being a 'Lewis' base)
- H+ + NH3 --> HNH3+
- Ag+ + 2NH3 --> Ag(NH3)2+
[As you can see the 'Lewis' definition is much wider than the 'Bronsted/Lowry': it needs free places for an electron pair, not H+]
What else can I help you with?
What kind of substance accepts an electron pair hydroxide ion alkali base acid?
A Lewis acid accepts an electron pair.
What kind of substance accepts an electron-pair?
The correct answer is acid.
How can one identify whether a substance is a Lewis acid or base?
A substance can be identified as a Lewis acid if it accepts an electron pair, and as a Lewis base if it donates an electron pair. Lewis acids are electron pair acceptors, while Lewis bases are electron pair donors.
Which substance accepts an electron pair?
A Lewis acid.
What substance accepts an electron pair?
The correct answer is acid.
Does The Lewis definition describes an acid as an electron-pair acceptor in a reaction true or false?
True. The Lewis definition of an acid describes it as a substance that can accept an electron pair, while a base is a substance that donates an electron pair.
What kind of substance accepts an electtom pair?
A substance that accepts an electron pair is called a Lewis acid. Lewis acids are typically electron-deficient species, such as metal cations or molecules with incomplete octets, that can form coordinate covalent bonds by accepting electron pairs from Lewis bases, which donate the pairs. This interaction is fundamental in many chemical reactions, including catalysis and complex formation.
What kind of substance accepts and electronics pair?
A substance that accepts an electron pair is known as a Lewis acid. Lewis acids are typically electron-deficient species that can form coordinate covalent bonds with electron-rich species, or Lewis bases, which donate an electron pair. Examples of Lewis acids include metal cations, certain nonmetals like boron trifluoride (BF3), and transition metal complexes. This interaction is fundamental in many chemical reactions, including catalysis and coordination chemistry.
What is the definition of Lewis Acids and Bases?
A Lewis acid is therefore any substance, such as the H+ ion, that can accept a pair of nonbonding electrons. In other words, a Lewis acid is an electron-pair acceptor. A Lewis base is any substance, such as the OH- ion, that can donate a pair of nonbonding electrons. A Lewis base is therefore an electron-pair donor.
What kind of substance accepts an electron?
The correct answer is acid.
What kind substance accepts electron pairs?
The correct answer is acid.
What kind of substance accepts electron pair?
As the definition of a Lewis acid says:"Capable of accepting electron pair (from a (Lewis) base".So H+ and Ag+ are both Lewis acids compared in the following reaction with ammonia:(in which the N-atom is donating the unbound electron pair as being a 'Lewis' base)H+ + NH3 --> HNH3+Ag+ + 2NH3 --> Ag(NH3)2+[As you can see the 'Lewis' definition is much wider than the 'Bronsted/Lowry': it needs free places for an electron pair, not H+]
